How many moles of gas must be forced into a 3.5 L ball to give it a gauge pressure of 9.4 psi at 25 degrees C? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is 14.7 psi so that the total pressure in the ball is 24.1 psi

Question

How many moles of gas must be forced into a 3.5 L ball to give it a gauge pressure of  9.4 psi at 25 degrees C? The gauge pressure is relative to atmospheric pressure. Assume that atmospheric pressure is 14.7 psi so that the total pressure in the ball is 24.1 psi
Ok so I'm doing PV=nRT solving for n. PV/RT

So I'm converting psi to atm  but I'm confused what is all the extra info given. Isn't it 9.4 psi / 14.7 psi x 1 atm

DrBob222 · Answer

No, if the gauge pressure is 9.4 then the pressure in the ball will be 14.7+9.4 psi = 24.1 psi and that's what the other information tells you. So 24.1 psi x (1 atm/14.7 psi) = ?atm Then n - PV/RT

Monique · Answer

Ahhhhh thank you!!!!! I was so frustrated

Anonymous · Answer

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Rhoda · Answer

Yes, this technique worked. I have how many moles of gas must be forced into a 4.0L ball to give it a pressure of 8.6 psi at 28C. Assume the atm is 14.8 psi so that the total pressure in the ball is 23.4psi
.0821*301.1/4*1.25=
6.36/24.74=.257